b) Identify how many moles of carbon dioxide would be released from the equation in (a) if 25.0 g of naphthalene were burned in the presence of excess oxygen.
This is the equation: C10H8 + 12 O2 → 10 CO2 + 4 H2O
also can you help with the next question. Its related to the question above.
c) Explain what would happen if only 1 mole of oxygen gas were available to interact with naphthalene in this reaction.
how many moles of C10H8 in 25g?
you will get 10 times that many moles of CO2
(c) you will use 1/12 mole of C10H8
So all I have to do is find the the number of moles in CO2 and multiply it by ten?
and then for c) can explain a little more what you did their so I can understand better.
the equation says that for every mole of C10H8 you get
10 moles of CO2
you use 12 moles of O2
To to ooblecks response:
C10H8 + 12 O2 → 10 CO2 + 4 H2O
If you know the number of moles in 25 g C10H8 the equation tells you that you get 10 mols CO2 for every 1 mol C10H8 burned.
For the question about using just 1 mol O2, the equation tells that every 1 mol C10H8 uses 12 mols O2; therefore, if you have just 1 mol O2 you can burn only 1/12 mol C10H8. I find that students often like to see the math so for the first one we have mols C10H8 = g/molar mass = 25/128 = 0.195, then mols CO2 = mols C10H8 x (10 mols CO2/1 mol C10H8) = 0.195 x 10/1 = ? Notice that mol C10H8 in the numberator cancel with mol C10H8 in the denominator to leave the answer in units of mols CO2 which is what you want. Applying this same reasoning to the second question you have
1 mol O2 x (1 mol C10H8/12 mol O2 = 1/12 mol C10H8. Notice that the units of O2 cancel to leave units of C10H8 which, again, is what you want for units in the answer.
To determine the number of moles of carbon dioxide released from the equation when 25.0 g of naphthalene is burned, we need to follow these steps:
Step 1: Calculate the molar mass of naphthalene.
The molar mass of naphthalene (C10H8) is the sum of the molar masses of carbon (C) and hydrogen (H) atoms in the compound. The molar mass of carbon is approximately 12.01 g/mol, and the molar mass of hydrogen is approximately 1.008 g/mol. Therefore:
Molar mass of C10H8 = (10 × molar mass of C) + (8 × molar mass of H)
Step 2: Convert the given mass of naphthalene to moles.
Use the formula: Number of moles = Mass / Molar mass
Step 3: Determine the stoichiometry ratio between naphthalene and carbon dioxide.
According to the balanced equation, for every 1 mole of naphthalene burned, 10 moles of carbon dioxide are produced.
Step 4: Multiply the moles of naphthalene by the stoichiometry ratio.
This calculation gives us the number of moles of carbon dioxide released.
Now, let's calculate the answer using the given information:
a) Molar mass of naphthalene:
Molar mass of C10H8 = (10 × molar mass of C) + (8 × molar mass of H) = (10 × 12.01 g/mol) + (8 × 1.008 g/mol) ≈ 128.18 g/mol
b) Number of moles of naphthalene:
Number of moles = Mass / Molar mass = 25.0 g / 128.18 g/mol ≈ 0.195 mol
c) Number of moles of carbon dioxide:
Number of moles of CO2 = Number of moles of naphthalene × (Stoichiometry ratio of CO2 / Stoichiometry ratio of naphthalene)
Number of moles of CO2 = 0.195 mol × (10 / 1) = 1.95 mol
Therefore, approximately 1.95 moles of carbon dioxide would be released when 25.0 g of naphthalene is burned in the presence of excess oxygen.
Now, let's move on to the next question:
c) If only 1 mole of oxygen gas were available to interact with naphthalene in this reaction, it would limit the reaction. Oxygen is in excess in the given equation, which means there is more than enough oxygen to react with the naphthalene. But if only 1 mole of oxygen gas is present, it is not enough to fully react with the naphthalene.
According to the stoichiometry of the balanced equation, 12 moles of oxygen gas (O2) are required to react with 1 mole of naphthalene (C10H8). However, if only 1 mole of oxygen gas is available, it means there isn't enough oxygen to fully react with the naphthalene.
In this case, the reaction will not be complete, and some naphthalene will remain unreacted or partially reacted. The unreacted or partially reacted naphthalene will not produce the expected amount of carbon dioxide and water as per the balanced equation.
It is important to have the balanced stoichiometry and enough reactants (in this case, oxygen gas) to ensure a complete and efficient reaction, leading to the expected amount of products.